i need to write to chemical formula for sulphur(II)iodide
but both are non metals what do i do
and i get confused sometimes cause i don't know when the metal/non metal gets a one charge (for the valences)
ex. NiO
=Ni1O2
=Ni2O
=Nickel(I)Oxide
ex.
NiF2
=Ni1F2
=Ni2F
=Nickel(II)Fluoride
(i don't know if that is correct or not so can you tell me if the valences are right or not and can you tell me how i get the valences for that specific element cause i don't understand where the valences are when it is one of the transition elements)
PLZ ANSWER ASAP cause i really need help for it :) :)
If you are given a name that has a metal with a multivalent possibility, the Roman numerals will tell you which to use. For nickel(I) oxide, that tells you Ni is I (i.e., +1) and not II (i.e., +2. the other common valence). Oxygen usually is -2 so you write Ni2O. For nickel(II) fluoride, that tells you to use Ni as +2 and the formula obviously is NiF2.
So for sulfur(II) iodide you would write
SI2. Sulfur(VI) fluoride would be SF6 (and that often is called sulfur hexafluoride). Post again if this isn't clear. Thanks for making your question very clear by using examples of what is troubling you.
so for all the chemical formulas if there is no subscript (for the valency of the element) does it mean it is a one or do i have to find the valency on the periodic table of elements?
ex. P02
the P for Phosphorus doesn't have a number does it mean it is a one then
ex.SO3
ex.FeCl3
ex.SnCl2
ex.Cu2O
ex.NiBr2
and can you check my answers for and can you tell me which ones are wrong and to correct it...
SnCl2 = Tin(II)Chloride
Cu2O = Copper(I)Oxide
NiBr2 = Nickel(II)Bromide
FeO = Iron(II) Oxide
SbBr5 = Antimony(V)Bromide
CoO = Cobalt(II)Oxide
MnF2 = Manganese(II)Fluoride
SnO2 = Tin(II)Oxide
SO2 = Tin(I)Oxide
BrF7 = Bromine(VI)Fluoride
1. Cobalt(II)Chloride = Co2Cl = CoCl2
2. Sulphur(II)Iodide = S2I1 = SI2
3. Iron(III)Chloride = Fe3Cl1= FeCl3
4. Antimony(V)Sulphide = Sb5S2 = Sb2S5
5. Lead(II)Nitride = Pb2N3 = Pb3N2
6. Tin(II)Fluoride = Sn2F1 = SnF2
7. Copper(II)Oxide = Cu2O2 = CuO
8. Tin(IV)Chloride = Sn4Cl1= SnCl4
9. Mercury(I)Phospide = Hg1P3 = Hg3P
i know that it is a lot of questions but i only put that many is because i am scared that i wont understand with only 1 or 2 examples if and when i am wrong so plz check and answer ASAP cause i need help for it
To write the chemical formula for sulphur(II)iodide, we need to determine the valences of both sulphur and iodine. Valence refers to the number of electrons an atom can gain, lose, or share to form a chemical bond.
Sulphur, which is a non-metal, typically has a valence of 2, meaning it can gain or share two electrons to form a bond. Iodine, another non-metal, usually has a valence of 1, meaning it can gain or share one electron to form a bond.
Now, let's combine these valences to write the chemical formula for sulphur(II)iodide.
Since sulphur has a valence of 2, we need two iodine atoms (each contributing one electron) to balance the charge. Therefore, the formula will be SI2.
It's important to note that when writing chemical formulas, we omit the "1" subscript for elements since it is unnecessary. So, there's no need to write SI2 as SI2.
Regarding your examples, let's review them:
1. NiO: Nickel(II)oxide - This is correct. Nickel typically has a valence of 2, which means it forms a 2+ charge. Oxygen has a valence of 2 and forms a 2- charge. Therefore, we need one nickel atom (Ni2+) and one oxygen atom (O2-) to balance the charges.
2. NiF2: Nickel(II)fluoride - This is also correct. Nickel forms a 2+ charge, and fluorine has a valence of 1, forming a 1- charge. Therefore, we need one nickel atom (Ni2+) and two fluorine atoms (2F1-) to balance the charges.
When dealing with transition elements like nickel, it's essential to consult the periodic table to determine the common valences. Transition metals can have multiple valences, so it's crucial to keep track of them.
Remember, if the compound is neutral (no overall charge), the sum of the charges of all the atoms in the chemical formula must be zero.